4. TemperatureDependencies 180 Understanding the high-temperature behavior of ni

Question

4. TemperatureDependencies 180
Understanding the high-temperature behavior of nitrogen oxides isessential for controlling pollution generated in automobileengines. The decomposition of nitric oxide (NO) to N2and O2 is second order with a rate constant of 0.0796M-1 s-1 at 737oC and 0.0815M-1 s-1 at 947oC. Calculate theactivation energy for the reaction (in kJ/mol). Give your answerusing 3 significant figures.


Please help me with this, I don't get howto solve it. It is a review and I don't remember :-/

Thanks!

Explanation / Answer

k = A*exp(-E/RT) k1 = A*exp(-E/R*T1) k2 = A*exp(-E/R*T2) ln(k1/k2) = (-E/R)*(1/T1 - 1/T2) k1 = 0.0796; k2 = 0.0815; T1 = 737 + 273 = 1000K    T2 = 947 + 273 = 1220K ln(0.0796 / 0.0815) = -(E/R) *(1/1000K - 1/1220K) E/R = 130.811 K R = 8.314 J/mol/K E = 1087.56536 J/mol ~ 1.09 kJ/mol

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